Imagine a 1.00 L container which initially contains 0.250 atm of H2O and CO each construct and complete an ICE table and determine the equilibrium concentrations of each gas
Solution:
The equilibrium reaction between CO and H2O using ICE table can be written as,
CO + H2O ==== CO2 + H2.
0.250 ---- 0.250 --------- 0 ---------- 0 atm (Initial)
-X -------- -X ---------------- + X ---------- + X atm (Change)
(0.250 - X)--(0.250 - X) --(X) -------X atm. ( Equilibrium)
Thus, equilbrium constant (Kp) is written as,
Kp = [CO2] [H2] / [CO] [H2O]
Kp = X . X / (0.250-X) ( 0.250-X)
Kp = X^2 / (0.250 - X) (0.250-X)
Therefore,
Equilibrium concentration of H2O, CO, H2 and CO2 are:
[H2O] = (0.250-X)
[CO] = (0.250 - X)
[CO2] = X
[H2] = X
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